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I know that equilibrium constant depends on temperature and concentration. But according to Le Chatelier's principle when we change concentration of reagents the equilibrium is the same. Why? |
I know that equilibrium constant depends on temperature and pressure. But according to Le Chatelier's principle when we change pressure of reagents the equilibrium is the same. Why? |
I am doing a chemistry lab report on figuring out the volume of air trapped inside a bottle. Here is the procedure:
1. Fill a larger container or tub about half full with tap water
2. Fill a 2 L plastic soft drink bottle with tap water. Put the cap on loosely
3. Carefully turn the bottle upside down without ... |
I am doing a chemistry lab report on figuring out the volume of air trapped inside a bottle. Here is the procedure:
1. Fill a larger container or tub about half full with tap water
2. Fill a 2 L plastic soft drink bottle with tap water. Put the cap on loosely
3. Carefully turn the bottle upside down without ... |
I found a site with this formalae if you will, Formal Charge = [# of valence electrons on atom] – [non-bonded electrons + number of bonds].
I don't think I am using it correctly in finding the formal charges of each atom in SO4(2-) S=2, O=-1 and the other O=0 and if you add them together I dont get the overall charge... |
I don't really like parts of this explanation (was hoping to find a better one here actually), but it's the best I know. I'll build on suggestions by @michielim and @vrtcl1dvoshun.
(Note: I think most of this argument can be transposed to the orbital overlap picture of bonding, but it might be slightly trickier to ... |
I don't really like parts of this explanation (was hoping to find a better one here actually), but it's the best I know. I'll build on suggestions by @michielim and @vrtcl1dvoshun.
(Note: I think most of this argument can be transposed to the orbital overlap picture of bonding, but it might be slightly trickier to ... |
good question here - the equilibrium constant is all a little bit abstract, and therefore tough for some of us chemists, at least initially :) I have always thought about the concept of 'equilibrium' in terms of a balloon.
Imagine a balloon, and you've blown the balloon up until it is as full as can be. At this stag... |
Certain reduction reactions require electrons as reducing agents. Then is the overlapping of orbits is necessary for electron transfer? I mean if a element X is heated and it gives out thermionic electrons then can an Oxidizing agent Y acquire it and get reduced? If so then will it acquire fast moving electrons or slow... |
I know this is broad so I will narrow:
Why does molten [PLA][1] stick to Aluminum?
I ask because I'm looking for a way to prevent/reduce the friction of the plastic inside the aluminum barrel of a 3D Printer. I believe that I can treat the surface of the aluminum with a High Temp enamel however I need to be sure of... |
Certain reduction reactions require electrons as reducing agents. Is the overlapping of orbitals is necessary for electron transfer? I mean if a element $\ce{X}$ is heated and it gives out thermionic electrons then can an oxidizing agent $\ce{Y}$ acquire it and get reduced? If so then will it acquire fast moving electr... |
The **position** of equilibrium depends on temperature and pressure, as Nick Burns describes in his answer. The equilibrium **constant** depends on temperature only. The equilibrium constant is not a measure of the position of equilibrium, but rather which positions (representing different compositions) along the the r... |
Your formula is correct. If $V$ is the number of valence electrons originally assigned to an atom, $N$ is the number of nonbonding electrons, and $B$ is the number of bonds ($\frac{1}{2}$ of the number of bonding electrons to be more precise), then the formal charge $FC$ is:
$$FC = V - (B+N)$$
Sulfate ion has two... |
I found a site with this formalae if you will,
Formal Charge = [# of valence electrons on atom] – [non-bonded electrons + number of bonds]
I don't think I am using it correctly in finding the formal charges of each atom in $\ce{SO_4\ ^{2-}}$. $\ce{S=2}$, $\ce{O=-1}$ and the other $\ce{O=0}$ and if you add them t... |
I found a site with this formalae if you will,
>Formal Charge = [# of valence electrons on atom] – [non-bonded electrons + number of bonds]
I don't think I am using it correctly in finding the formal charges of each atom in $\ce{SO_4^{2-}}$. $\ce{S=2}$, $\ce{O=-1}$ and the other $\ce{O=0}$ and if you add them to... |
I found a site with this formalae if you will,
>Formal Charge = [# of valence electrons on atom] – [non-bonded electrons + number of bonds]
I don't think I am using it correctly in finding the formal charges of each atom in $\ce{SO_4^{2-}}$. $\ce{S}=2$, $\ce{O}=-1$ and the other $\ce{O}=0$ and if you add them to... |
Why is it that the extent of racemisation is greater in $S_N 1$ reaction caried out using polar protic solvent but the racemisation is not as extensive if aprotic solvent is used although the carbocation intermediate is common in both?
eg:- 2-Bromobutane is solvolysed with $\ce{H2O}$ and $\ce{CH3OH}$ but the racemi... |
Relative racemisation in $S_N 1$ reaction? |
How do I find partial pressures if I am only given their percentages? where do I begin?
eg.
O=21% , N=78% , Ar=1% by volume how would I calcluate the partial pressures if total pressure is 1atm. |
A binary compound, of lead and oxygen contains 90.66% Pb, what is the empirical formula for the compound?
How do i use to percentage to get to the regular formula, then how do I change the normal formula to empirical? |
Empirical formula when given percentages? |
You will get the empirical formula straight from this data. In order to convert to a molecular formula, you need more information.
By way of another example:
> A binary compound of tin and chlorine contains 62.89% tin by mass. Determine the empirical formula.
Our first goal is to figure out the ratio of *moles... |
Your formula is correct. If $V$ is the number of valence electrons originally assigned to an atom, $N$ is the number of nonbonding electrons, and $B$ is the number of bonds ($\frac{1}{2}$ of the number of bonding electrons to be more precise), then the formal charge $FC$ is:
$$FC = V - (B+N)$$
Sulfate ion has two... |
So I did for my AS Level exam today a titration experiment, seeing how much sulfuric acid of (I think) about $0.100 - 0.200 mol dm^-3$, which went in the burette, is needed to react with 0.1M sodium hydroxide, in the conical flask.
We lose a mark for every $0.10cm^3$ we are off of the actual titre value that should... |
What is the titre of a sodium hydroxide-sulfuric acid titration experiment? |
So I did for my AS Level exam today a titration experiment, seeing how much sulfuric acid of (I think) about $0.100 - 0.200 \text{ mol dm}^-3$, which went in the burette, is needed to react with 0.1M sodium hydroxide, in the conical flask.
We lose a mark for every $0.10\text{ cm}^3$ we are off of the actual titre v... |
My textbook, *Organic Chemistry* (6th edition) by Brown, Foote, Iverson, and Anslyn, states:
> Alkynes in which the triple bond is between carbons 1 and 2 are commonly referred to as **terminal alkynes**.
Is not this definition incomplete? I can imagine scenarios where we have a terminal triple bond that does not r... |
Correct definition of terminal alkynes? |
Maybe this is better in English.SE, but I think I'm more likely to get better responses here in the "industry" site. [This post][1] got me thinking; how do you pronounce "alkyne" (a hydrocarbon with a carbon-carbon *triple* bond) differently enough from "alkene" (a hydrocarbon with a carbon-carbon *double* bond) to dif... |
English isn't my first language, and in truth I'm always doubtful about the pronunciation of words in chemistry. Sometimes it's possible to find videos where the words are mentioned, for example [here][1] or [here][2] or [here][3]. That's what I use, al-keen and al-kyne (ky as in kite or sky).
[1]: https://www.y... |
English isn't my first language, and in truth I'm always doubtful about the pronunciation of words in chemistry. Sometimes it's possible to find videos where the words are mentioned, for example [here][1] or [here][2] or [here][3] or [here][4] (several examples of alkenes and alkynes being pronounced in this last one).... |
How many lbf/in^2 need to break JB weld? |
How many $\text{lbf}/\text{in}^2$ need to break JB weld? |
So I did for my AS Level exam today a titration experiment, seeing how much sulfuric acid of (I think) about $0.100 - 0.200 \text{ mol dm}^{-3}$, which went in the burette, is needed to react with 0.1M sodium hydroxide, in the conical flask.
We lose a mark for every $0.10\text{ cm}^3$ we are off of the actual titre... |
[Thermal Grease][1] is used to remove the air gaps between CPU and heatsink. However, computing aside, what would determine the max temp that the grease can handle before it burns or breaks down?
[1]: https://en.wikipedia.org/wiki/Thermal_grease |
How hot can Thermal Grease get? |
JB Weld, a brand name of steel-reinforced epoxy, makes claims of being the "world's strongest bond".
What is the maximum pressure it can withstand, and what is it about the interaction between the steel and the epoxy that makes it so strong? |
What is the maximum pressure that JB Weld can withstand? |
I'm no chemist, but much of my work revolves around biochar. I've always understood it with the following rough approximation:
$$CH_2O + heat \rightarrow BC + H_2 + CO + CH_4 + HC's$$
where the first term approximates dry plant matter, BC is black carbon, and "HC's" represent various heavy hydrocarbons.
I've ... |
For example, $\ce{CH_2CHBrCH_3}$ reacts with $\ce{:NH_3}$ to make $\ce{CH_2C^+H(NH_3)CH_3 +:Br^-}$, then reacting again with $\ce{:NH_3}$ to make $\ce{CH_2CH(NH_2)CH_3 +:Br^- +CH_4^+}$.
Question: why does the last step not produce $\ce{CH_2CH(NH_2)CH_3 +HBr}$? That is, why is Ammonia a better nucleophile than the ... |
Why does nucleophilic substitution of a haloalkane with ammonia produce ammonium, not a hydrogen halide? |
For example, $\ce{CH3CHBrCH3}$ reacts with $\ce{:NH_3}$ to make $\ce{CH3CH(NH3^+)CH3 +:Br-}$, then reacting again with $\ce{:NH_3}$ to make $\ce{CH3CH(NH2)CH3 +:Br^- +NH4^+}$.
Question: why does the last step not produce $\ce{CH3CH(NH2)CH3 +HBr}$? That is, why is Ammonia a better nucleophile than the halide ion, d... |
I'm studying for my chemistry final and having a hard time with this question on one of the practice exams. Here's the question:
At $20$ degreees Celsius, Henry's Law constant for Ar is half of that for Kr. If a gaseous Ar/Kr mixture containing molar fraction of Kr is placed over water at $20$ degrees Celcius, what ... |
I'm studying for my chemistry final and having a hard time with this question on one of the practice exams. Here's the question:
At $20$ degreees Celsius, Henry's Law constant for Ar is half of that for Kr. If a gaseous Ar/Kr mixture containing 20% molar fraction of Kr is placed over water at $20$ degrees Celcius, w... |
For example, $\ce{CH3CHBrCH3}$ reacts with $\ce{:NH_3}$ to make $\ce{CH3CH(NH3^+)CH3 +:Br-}$,$$\ce{CH3CHBrCH3 \rightarrow CH3CH(NH3^+)CH3 +:Br-}$$then reacting again with $\ce{:NH_3}$ to make $\ce{CH3CH(NH2)CH3 +:Br^- +NH4^+}$:
$$\ce{NH_3 + CH3CH(NH3^+)CH3 +:Br- \rightarrow CH3CH(NH2)CH3 +:Br^- +NH4^+} $$
Questi... |
Why is the complex $\ce{[FeCl4]-}$ stronger than $\ce{[CuCl4]-}$ and $\ce{[CoCl4]-}$? And why won't $\ce{Ni^2+}$ form a complex with $\ce{Cl-}$?
According to the HSAB theory, $\ce{Cl-}$ is considered a hard/borderline base. So I figured the strongest complex would be the one in which the center ion is the hardest ac... |
The link to your handout explains why $\ce{Fe^{3+}}$ (and it is $\ce{Fe^{3+}}$ in $\ce{FeCl4^{-}}$) is a harder acid than $\ce{Co^{3+}}$ or $\ce{Cu^{2+}}$ or $\ce{Ni^{2+}}$.
>Hard acids (in context, HA) are characterized by (s,f blocks, **left side of d block** in higher OS's)
Iron is the furthest to the left of ... |
Why won't $\ce{Ni^2+}$ form a complex with $\ce{Cl-}$, while the ions $\ce{Cu^2+}$ and $\ce{Co^2+}$ form the complexes $\ce{[CuCl4]^2-}$ and $\ce{[CoCl4]^2-}$?
According to the HSAB theory, $\ce{Cl-}$ is considered a hard/borderline base. So I figured the strongest complex would be the one in which the center ion ... |
In the TV show "Breaking Bad", Walter White frequently gets rid of people who get in his way by submerging them in a plastic container full of hydrofluoric acid. This, at least in the TV show, completely dissolves the body leaving nothing but a red sludge behind at the end.
Is it actually possible to dispose of a bo... |
Is it actually possible to dispose of a body with hydrofluoric acid? |
[XKCD #1162][1] piqued my curiosity. Obviously, there's nothing we generally use for fuel that can match the energy density of uranium fission. But I wondered what it would take, hypothetically, to match it mole-for-mole?
Looking at the [bond enthalpy charts][2], I see that the carbon-oxygen triple bond has the high... |
[XKCD #1162][1] piqued my curiosity. Obviously, there's nothing we generally use as a chemical fuel that can match the energy density of uranium fission. But I wondered what it would take, hypothetically, to match it mole-for-mole?
Looking at the [bond enthalpy charts][2], I see that the carbon-oxygen triple bond ha... |
Getting a large exotherm per mole of molecules is a bit of a bad cheat if you're allowed to make molecules arbitrarily big! Energy per mass is the only honest way to do it. However, there really is no way to chemically match a nuclear exotherm in any honest way, nuclear energies are simply in a class of their own.
... |
Getting a large exotherm per mole of molecules is a bit of a bad cheat if you're allowed to make molecules arbitrarily big! Energy per mass is the only honest way to do it. However, there really is no chance to chemically match a nuclear exotherm; nuclear energies are simply in a class of their own.
Practically all... |
Getting a large exotherm per mole of molecules is a bit of a bad cheat if you're allowed to make molecules arbitrarily big! Energy per mass is the only honest way to do it (or energy per mole of atoms would work too I guess). However, there really is no chance to chemically match a nuclear exotherm; nuclear energies ar... |
A proper answer to your question would require at least a semester of Physical Chemistry. I would like to touch on a couple of issues (very loosely speaking):
- We know from quantum mechanics that electrons have certain properties, which are couched in something called a wave function. Mathematically, wave functio... |
It is extremely difficult to look at a molecule and know whether it is explosive.
Generally speaking, highly exothermic chemical reactions are the "explosive" ones.
A --> B + C
What makes the reaction exothermic? Either A is very unstable, or B and C are very stable. Any molecule that has lots of very stable... |
It is extremely difficult to look at a molecule and know whether it is explosive.
But, generally speaking, highly exothermic chemical reactions are the "explosive" ones.
A --> B + C
What makes the reaction exothermic? Either A is very unstable, or B and C are very stable. Any molecule that has lots of very s... |
The real issue is that no one has ever taken a picture (i.e. electron density) of genuine, unambigious, cases of a single, double, triple, quadruple??? bonds. And they never will, because these concepts are not based on quantum mechanics.
Two atoms reside next to each other, and if they have a favorable electrostati... |
The real issue is that no one has ever taken a picture (i.e. electron density) of genuine, unambigious, cases of a single, double, triple, quadruple??? bonds. And they never will, because these concepts are not based on quantum mechanics.
Two atoms reside next to each other, and if they have a favorable electrostati... |
I was reading [this question and the answer by @EricBrown][1] to it and this got me thinking about covalent chemical bonds.
The way I was always taught is that a single bond contains 2 paired electrons, a double bond 4 etc ([The Lewis dots drawings][2] always show this nicely). In his answer Eric mentions that the ... |
Electron density definition of single, double, triple bonds? |
The answer is that there is one (or perhaps two) types of bonds. A _bond_ occurs when two atoms are attracted in a net-electrostatically favorable way. (Of course, the electrons and protons are subject to their quantum nature)
Why two? In the Quantum Theory of Atoms in Molecules, the "procedure" is:
1. Ascertai... |
The answer is that there is one (or perhaps two) types of bonds. A _bond_ occurs when two atoms are attracted in a net-electrostatically favorable way. (Of course, the electrons and protons are subject to their quantum nature)
Why two? In the [Quantum Theory of Atoms in Molecules][1], the "procedure" is:
1. Asc... |
The answer is that there is one (or perhaps two) types of bonds. A _bond_ occurs when two atoms are attracted in a net-electrostatically favorable way. (Of course, the electrons and protons are subject to their quantum nature)
Why two? In the [Quantum Theory of Atoms in Molecules][1], the "procedure" is:
1. Asc... |
The answer is that there is one (or perhaps two) types of bonds. A _bond_ occurs when two atoms are attracted in a net-electrostatically favorable way. (Of course, the electrons and protons are subject to their quantum nature)
Why two? In the [Quantum Theory of Atoms in Molecules][1], the "procedure" is:
1. Asc... |
So I'm carrying out the distillation of some essential oil and I have to remove the water content in it. The usual method is using diethyl ether but I'm looking for a greener method.
What can I do ? |
how do you calculate the wavelength of light? For chemsitry lab, we calibrated the scale reading of Hg, for example, to be 4.91 cm which is violet and the given wavelength says 436. For Hg, it says scale reading of 5.51 cm for green and wavelength of 546. But for overhead fluorescent, I took the scale reading of 4.93 ... |
Below are plots of the electron density for ethane, ethene, and ethyne. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal plane that still contains the two carbon atoms.
A co... |
Below are plots of the electron density for ethane, ethene, and ethyne. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal plane that still contains the two carbon atoms.
A co... |
Below are plots of the electron density for staggered ethane, ethene, and ethyne. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal plane that still contains the two carbon atom... |
Below are plots of the electron density for staggered ethane, ethene, and ethyne. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal plane that still contains the two carbon atom... |
Below are plots of the electron density for staggered ethane, ethene, and ethyne, computed from electronic structure theory. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal pl... |
(Fairness in reporting: I am a hard-core Quantum Theory of Atoms in Molecules partisan)
NBO is one of many attempts the apply rotations among molecular orbitals, each of which can spread over the entire molecule, (i.e. the wave function) so that they maximally-resemble localized atomic orbitals or "hybrid atomic orb... |
Consider this reaction. :-
CaCO3(s) → CaO(s) + CO2(g)
for this, Kc=[ CO2(g)]
For a given temperature, Kc will remain fixed. That means, the amount of CO2 released will be same, irrespective of amount of CaCO3 taken.
But,that means , at the same temperature,irrespective of whether we start with 1gm of C... |
Consider this reaction. :-
\ce{N2(g) + 3H2(g) <=>2NH3(g)}
for this, Kc=[ CO2(g)]
For a given temperature, Kc will remain fixed. That means, the amount of CO2 released will be same, irrespective of amount of CaCO3 taken.
But,that means , at the same temperature,irrespective of whether we start with ... |
Consider this reaction. :-
$CaCO_3$(s) → $CaO$(s) + $CO_2$(g)
for this, Kc=[ $CO_2$ g)]
For a given temperature, Kc will remain fixed. That means, the amount of $CO_2$ released will be same, irrespective of amount of $CaCO_3$ taken.
But,that means , at the same temperature,irrespective of whether ... |
Consider this reaction. :-
**$CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$**
for this, Kc=[ $CO_2$ g)]
For a given temperature, Kc will remain fixed. That means, the amount of $CO_2$ released will be same, irrespective of amount of $CaCO_3$ taken.
But,that means , at the same temperature,irre... |
If I mix Cysteine powder in Juice (something acidic maybe), does it remain at Cysteine?
It seems that it can oxidize into Cystine and loose some of its qualities. Is it preferred to cap it and let is break apart directly in stomach acid?
|
What is the best way to disolve and consume Cysteine HCL Monohydrate powder? |
If I mix Cysteine powder in Juice (something acidic maybe), does it remain at Cysteine?
It seems that it can oxidize into Cystine and loose some of its qualities. Veg-caps deliver the powder directly to the stomach acid. What might be a good alternative way to drink it without the trouble and expense of cappin... |
Below are plots of the electron density for staggered ethane, ethene, and ethyne, computed from electronic structure theory. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal pl... |
Why is that in an external magnetic field(uniform) the degeneracy of d,f orbitals is lost but the degeneracy of p orbitals remain intact if the main cause of losing degeneracy is the difference in energy of differently oriented orbitals in the magnetic field? |
Degeneracy of orbitals? |
I am not able to find any examples of inductive effect operating through multiple bonds . Why can't electron displacement take place in multiple bonds ? |
Why Inductive effect operates only through single bonds? |
Consider this reaction. :-
**$CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$**
for this, Kc=[ $CO_2$ g)]
For a given temperature, Kc will remain fixed. That means, the amount of $CO_2$ released will be same, irrespective of amount of $CaCO_3$ taken.
But,that means , at the same temperature,irre... |
a balloon is half filled with water at sea level (P = 1 atm, T = 298K) such that partial pressure of water is 24 mmHg. its then submerged to a point where P = 2 atm, T = 298K. what will be the vapor pressure of water at that point?
my first instinct is to find the mole fraction of water in the balloon. using dalt... |
A balloon is half filled with water at sea level ($P = 1$ atm, $T = 298$K) such that the partial pressure of water is $24$ mmHg. It is then submerged to a point where $P = 2$ atm, $T = 298$K. what will be the vapor pressure of water at that point?
My first instinct is to find the mole fraction of water in the ball... |
We know that the Michaelis Menten derivation for the following reaction:
E + S <-> ES -> E + P
Howver, what if the reaction took place in a different scenario whereby:
E + S <-> ES1 -> ES2 -> E + P
What would be the derived Michaelis Menten Equation now? |
Below are plots of the electron density for staggered ethane, ethene, and ethyne, computed from electronic structure theory. For ethene, which is planar, imagine that the hydogens are jutting forward and backward into the paper, so that the contour plots should contain any putative $\pi$ bonds. It is the orthogonal pl... |
First, as kaliaden commented, the true equilibrium constant
$$K(T,p) = a(\textrm{CaO,s}) a(\textrm{CO$_2$,g}) / a(\textrm{CaCO$_3$,s}) \approx
p_\textrm{CO$_2$} / p^\circ \equiv K_p(T)$$
where $a$ are the activities, $p$ the partial pressure and $p^\circ$ is one bar.
Thus $K$ basically only depends on temperatu... |
(Fairness in reporting: I am a hard-core Quantum Theory of Atoms in Molecules partisan)
NBO is one of many attempts the apply rotations among molecular orbitals, each of which can spread over the entire molecule, (i.e. the wave function) so that they maximally-resemble localized atomic orbitals or "hybrid atomic orb... |
We know that the Michaelis Menten derivation for the following reaction:
$\ce{E + S \rightleftharpoons ES -> E + P}$
Howver, what if the reaction took place in a different scenario whereby:
$\ce{E + S \rightleftharpoons ES1 -> ES2 -> E + P}$
What would be the derived Michaelis Menten Equation now? |
[XKCD #1162][1] piqued my curiosity. Obviously, there's nothing we generally use as a chemical fuel that can match the energy density of uranium fission. But I wondered what it would take, hypothetically, to match it mole-for-mole?
Looking at the [bond enthalpy charts][2], I see that the carbon-oxygen triple bond ha... |
I'm looking for a reducing sugar such as glucose or maltose (any reducing sugar will do) for some home chemistry experiments. Is there a readily available reducing sugar that I might source without contacting a chemical company? A simple "synthesis" of glucose from sucrose would work as well. |
How To Obtain A Reducing Sugar At Home? |
In [an article][1] I am trying to understand the following occurs:
>Synthesis of octahedral Cu2O seeds:In a typical synthesis, 2.9946 g of Cu(CH3COO)2 was dissolved in deionizedwater (20 mL) using a beaker under a constant stirring at 70°C for 2 min. A dark precipitate was produced when a sodium hydroxide solution ... |
How Do Octahedral Seed Crystals Yeild Polyhedral Cu2O Crystals? |
I read a paper about enzyme catalysed synthesis of octanamide (DOI: 10.1039/C39930001831).
What is octanamide used for? |
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